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General Certificate of Education
Advanced Subsidiary Examination
June 2015
Chemistry
Unit 2
CHEM2
Chemistry in Action
Tuesday 2 June 2015
Mark
1
2
3
4
5
6
1.30 pm to 3.15 pm
7
For this paper you must have:
 the Periodic Table/Data Sheet, provided as an insert
(enclosed)
 a ruler with millimetre measurements
 a calculator.
8
9
TOTAL
Time allowed
 1 hour 45 minutes
Instructions
 Use black ink or black ball-point pen.
 Fill in the boxes at the top of this page.
 Answer all questions.
 You must answer the questions in the spaces provided. Do not write
outside the box around each page or on blank pages.
 All working must be shown.
 Do all rough work in this book. Cross through any work you do not
want to be marked.
Information
 The marks for questions are shown in brackets.
 The maximum mark for this paper is 100.
 You are expected to use a calculator, where appropriate.
 The Periodic Table/Data Sheet is provided as an insert.
 Your answers to the questions in Section B should be written in
continuous prose, where appropriate.
 You will be marked on your ability to:
– use good English
– organise information clearly
– use scientific terminology accurately.
Advice
 You are advised to spend about 1 hour 15 minutes on Section A and
about 30 minutes on Section B.
(JUN15CHEM201)
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CHEM2
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Section A
Answer all questions in the spaces provided.
1
Chlorine is an important industrial chemical.
1 (a)
Chlorine is formed when KMnO4 reacts with hydrochloric acid.
The ionic equation for this redox reaction is
16H+ + 2MnO4– + 10Cl–
1 (a) (i)
2Mn2+ + 8H2O + 5Cl2
Deduce the half-equation for the oxidation of chloride ions to chlorine.
[1 mark]
.............................................................................................................................................
1 (a) (ii) Give the oxidation state of manganese in the MnO4– ion.
[1 mark]
.............................................................................................................................................
1 (a) (iii) Deduce the half-equation for the reduction of the MnO4– ions in acidified solution to
manganese(II) ions and water.
[1 mark]
.............................................................................................................................................
1 (b)
Chlorine behaves as an oxidising agent in the extraction of bromine from seawater.
In this process, chlorine gas is bubbled through a solution containing bromide ions.
1 (b) (i)
Write the simplest ionic equation for the reaction of chlorine with bromide ions.
[1 mark]
.............................................................................................................................................
1 (b) (ii) Give one observation that would be made during this reaction.
[1 mark]
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1 (b) (iii) In terms of electrons, state the meaning of the term oxidising agent.
[1 mark]
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1 (c)
In sunlight, chlorine can also oxidise water slowly to form oxygen.
Write an equation for this reaction.
Give the oxidation state of chlorine in the chlorine-containing species that is formed.
[2 marks]
Equation
.............................................................................................................................................
Oxidation state of chlorine in the species formed ..............................................................
1 (d)
Explain why chlorine has a lower boiling point than bromine.
[2 marks]
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2
The following pairs of compounds can be distinguished by simple test-tube reactions.
For each pair of compounds, give a reagent (or combination of reagents) that, when
added separately to each compound, could be used to distinguish between them.
State what is observed in each case.
2 (a)
Butan-2-ol and 2-methylpropan-2-ol
[3 marks]
Reagent ..............................................................................................................................
Observation with butan-2-ol
.............................................................................................................................................
.............................................................................................................................................
Observation with 2-methylpropan-2-ol
.............................................................................................................................................
.............................................................................................................................................
2 (b)
Propane and propene
[3 marks]
Reagent ...............................................................................................................................
Observation with propane
.............................................................................................................................................
.............................................................................................................................................
Observation with propene
.............................................................................................................................................
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2 (c)
Aqueous silver nitrate and aqueous sodium nitrate
[3 marks]
Reagent ..............................................................................................................................
Observation with aqueous silver nitrate
.............................................................................................................................................
.............................................................................................................................................
Observation with aqueous sodium nitrate
.............................................................................................................................................
.............................................................................................................................................
2 (d)
Aqueous magnesium chloride and aqueous barium chloride
[3 marks]
Reagent ..............................................................................................................................
Observation with aqueous magnesium chloride
.............................................................................................................................................
.............................................................................................................................................
Observation with aqueous barium chloride
.............................................................................................................................................
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3
The elements in Group 2 from Mg to Ba can be used to show the trends in properties
down a group in the Periodic Table.
3 (a)
State the trend in atomic radius for atoms of the elements down Group 2 from Mg to Ba
Give a reason for this trend.
[2 marks]
Trend ...................................................................................................................................
Reason ................................................................................................................................
.............................................................................................................................................
.............................................................................................................................................
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3 (b)
The Group 2 elements react with water.
3 (b) (i)
State the trend in reactivity with water of the elements down Group 2 from Mg to Ba
[1 mark]
.............................................................................................................................................
3 (b) (ii) Write an equation for the reaction of strontium with water.
[1 mark]
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3 (c)
Give the formula of the hydroxide of the element in Group 2 from Mg to Ba that is most
soluble in water.
[1 mark]
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5
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4
Hydrogen is produced in industry from methane and steam in a two-stage process.
4 (a)
In the first stage, carbon monoxide and hydrogen are formed.
The equation for this reaction is
CH4(g) + H2O(g)
4 (a) (i)
CO(g) + 3H2(g)
ΔH = +206 kJ mol–1
Use Le Chatelier’s principle to state whether a high or low temperature should be used
to obtain the highest possible equilibrium yield of hydrogen from this first stage.
Explain your answer.
[3 marks]
Temperature ........................................................................................................................
Explanation .........................................................................................................................
.............................................................................................................................................
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4 (a) (ii) Le Chatelier’s principle suggests that a high pressure will produce a low yield of
hydrogen in this first stage.
Explain, in terms of the behaviour of particles, why a high operating pressure is used in
industry.
[2 marks]
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4 (a) (iii) A nickel catalyst is used in the first stage.
Explain why the catalyst is more effective when coated onto an unreactive honeycomb.
[2 marks]
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4 (b)
The second stage is carried out in a separate reactor. Carbon monoxide is converted
into carbon dioxide and more hydrogen is formed.
The equation for this reaction is
CO(g) + H2O(g)
CO2(g) + H2(g)
ΔH = –41 kJ mol–1
Use Le Chatelier’s principle to state the effect, if any, of a decrease in the total pressure
on the yield of hydrogen in this second stage. Explain your answer.
[2 marks]
Effect ...................................................................................................................................
Explanation .........................................................................................................................
.............................................................................................................................................
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5
There are many uses of halogenated organic compounds despite environmental
concerns.
5 (a)
Bromotrifluoromethane is used in fire extinguishers in aircraft.
Bromotrifluoromethane is formed when trifluoromethane reacts with bromine.
CHF3 + Br2
CBrF3 + HBr
The reaction is a free-radical substitution reaction similar to the reaction of methane with
chlorine.
5 (a) (i)
Write an equation for each of the following steps in the mechanism for the reaction of
CHF3 with Br2
[4 marks]
Initiation step
.............................................................................................................................................
First propagation step
.............................................................................................................................................
Second propagation step
.............................................................................................................................................
A termination step
.............................................................................................................................................
5 (a) (ii) State one condition necessary for the initiation of this reaction.
[1 mark]
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5 (b)
Bromine-containing and chlorine-containing organic compounds may have a role in the
decomposition of ozone in the upper atmosphere.
5 (b) (i)
Draw an appropriate displayed formula in the space provided to complete the following
equation to show how CBrF3 may produce bromine atoms in the upper atmosphere.
[1 mark]
CBrF3
+
Br
...............................
5 (b) (ii) In the upper atmosphere, it is more likely for CBrF3 to produce bromine atoms than it is
for CClF3 to produce chlorine atoms.
Suggest one reason for this.
[1 mark]
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5 (b) (iii) Bromine atoms have a similar role to chlorine atoms in the decomposition of ozone.
The overall equation for the decomposition of ozone is
2O3
3O2
Write two equations to show how bromine atoms (Br) act as a catalyst in the
decomposition of ozone.
Explain how these two decomposition equations show that bromine atoms behave as a
catalyst.
[3 marks]
Equation 1
.............................................................................................................................................
Equation 2
.............................................................................................................................................
Explanation .........................................................................................................................
.............................................................................................................................................
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6
Butane and propanal are compounds with Mr = 58.0, calculated using data from your
Periodic Table.
6 (a)
A mass spectrometer can be used to distinguish between samples of butane and
propanal.
Table 1 shows some precise relative atomic mass values.
Table 1
Atom
6 (a) (i)
Precise relative atomic mass
1H
1.00794
12C
12.00000
Use data from Table 1 to show that, to 3 significant figures, a more accurate value for
the Mr of butane is 58.1
[1 mark]
.............................................................................................................................................
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6 (a) (ii) State why the precise relative atomic mass quoted in Table 1 for the 12C isotope is
exactly 12.00000
[1 mark]
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6 (b)
Draw a displayed formula for the organic product that is formed when propanal is
oxidised by warm Tollens’ reagent.
[1 mark]
6 (c)
Prop-2-en-1-ol is an isomer of propanal and can be polymerised to form a polymer
represented by the following structure.
( )
6 (c) (i)
H
CH2OH
C
C
H
H
n
Draw the structure of prop-2-en-1-ol.
[1 mark]
6 (c) (ii) Deduce the type of polymerisation that results in the formation of this polymer from
prop-2-en-1-ol.
[1 mark]
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6 (c) (iii) There are two functional groups in prop-2-en-1-ol. Each of these functional groups
contains a bond with a characteristic absorption range in the infrared spectrum.
Use Table A on the Data Sheet to suggest a bond and its absorption range for each of
the two functional groups.
[2 marks]
Bond 1 ............................ Absorption range ......................................................................
Bond 2 ............................ Absorption range ......................................................................
6 (d)
Compound X is another isomer of propanal. The infrared spectrum of X shows an
absorption in the range 1680–1750 cm–1.
6 (d) (i)
Draw the structure of X.
[1 mark]
6 (d) (ii) Which of the following, A, B, C or D, represents the type of isomerism shown by X and
propanal?
Write the correct letter, A, B, C or D, in the box.
[1 mark]
A
B
C
D
chain isomerism
E–Z isomerism
functional group isomerism
position isomerism
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7 (a)
Propanone can be formed when glucose comes into contact with bacteria in the
absence of air.
7 (a) (i)
Balance the following equation for this reaction of glucose to form propanone, carbon
dioxide and water.
[1 mark]
..........C6H12O6
..........CH3COCH3 + ..........CO2 + ..........H2O
7 (a) (ii) Deduce the role of the bacteria in this reaction.
[1 mark]
.............................................................................................................................................
7 (b)
Propanone is also formed by the oxidation of propan-2-ol.
7 (b) (i)
Write an equation for this reaction using [O] to represent the oxidising agent.
[1 mark]
.............................................................................................................................................
7 (b) (ii) State the class of alcohols to which propan-2-ol belongs.
[1 mark]
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7 (c)
A student determined a value for the enthalpy change when a sample of propanone was
burned. The heat produced was used to warm some water in a copper calorimeter.
The student found that the temperature of 150 g of water increased by 8.0 ºC when
4.50 × 10–3 mol of pure propanone was burned in air.
Use the student’s results to calculate a value, in kJ mol–1, for the enthalpy change when
one mole of propanone is burned.
(The specific heat capacity of water is 4.18 J K–1 g–1)
[3 marks]
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7 (d)
Define the term standard enthalpy of combustion.
[3 marks]
.............................................................................................................................................
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7 (e)
Use the mean bond enthalpy data in Table 2 and the equation given below Table 2 to
calculate a value for the standard enthalpy change when gaseous propanone is burned.
[3 marks]
Table 2
Mean bond enthalpy
/ kJ mol–1
C–H
C–C
C–O
O–H
C=O
O=O
412
348
360
463
805
496
CH3COCH3(g) + 4O2(g)
3CO2(g) + 3H2O(g)
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7 (f)
Suggest two reasons why the value obtained by the student in Question 7 (c) is different
from the value calculated in Question 7 (e).
[2 marks]
Reason 1 .............................................................................................................................
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Reason 2 .............................................................................................................................
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Section B
Answer all questions in the spaces provided.
8
Consider the following scheme of reactions.
CH3
H3C
C
CH3
Reaction 1
CH
CH3
CH2
H3C
Reaction 3
C
CHCl
CH3
CH3
P
Q
Reaction 2
CH3
H3C
C
CH(NH2)
CH3
CH3
R
8 (a)
Give the IUPAC name for compound P and that for compound Q.
[2 marks]
P ..........................................................................................................................................
Q .........................................................................................................................................
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8 (b)
The conversion of P into Q in Reaction 1 uses HCl
Name and outline a mechanism for this reaction.
[5 marks]
.............................................................................................................................................
8 (c)
The conversion of Q into R in Reaction 2 uses NH3
Name and outline a mechanism for this reaction.
[5 marks]
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8 (d)
State the type of reaction shown by Reaction 3.
Identify a reagent for this reaction.
Give one condition necessary for a high yield of product when Q is converted into P.
[3 marks]
.............................................................................................................................................
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8 (e)
Hydrogen bromide (HBr) could be used in the overall conversion of P into R, instead of
using HCl
Hydrogen bromide is made by the reaction of NaBr with concentrated phosphoric acid.
Concentrated sulfuric acid is not used to make HBr from NaBr
Write an equation for the reaction of NaBr with H3PO4 to produce HBr and Na3PO4 only.
Identify two toxic gases that are formed, together with HBr, when NaBr reacts with
concentrated H2SO4
State the role of H2SO4 in the formation of these two toxic gases.
[4 marks]
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9
Vanadium is an important metal. Ferrovanadium, an alloy of iron and vanadium, is used
to make a strong type of vanadium-steel. Pure vanadium is used in nuclear reactors.
9 (a)
Table 3 shows some standard enthalpy of formation data.
Table 3
ΔHf / kJ mol–1
V2O5(s)
CaO(s)
–1560
–635
In the oldest method of extraction of vanadium, V2O5 is reacted with calcium at a high
temperature.
5Ca(s) + V2O5(s)
2V(s) + 5CaO(s)
Use data from Table 3 and the equation to calculate the standard enthalpy change for
this reaction.
State the type of reaction that V2O5 has undergone.
Suggest one major reason why this method of extracting vanadium is expensive, other
than the cost of heating the reaction mixture.
[5 marks]
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9 (b)
Ferrovanadium is produced by the reaction of aluminium with a mixture of V2O5 and
iron(III) oxide.
Write an equation for the reaction of aluminium with iron(III) oxide.
State the change in oxidation state of aluminium in this reaction.
[2 marks]
.............................................................................................................................................
.............................................................................................................................................
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9 (c)
Pure vanadium, for nuclear reactors, is formed by the reaction of hydrogen with purified
VCl2
Write an equation for this reaction in which the only other product is HCl gas.
Identify two hazards in this process, other than the fact that it operates at a high
temperature.
Deduce why this process produces pure vanadium, other than the fact that purified
VCl2 is used.
[4 marks]
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